Study guide for Exam 3 Chem 1212 Fall 2
Study guide for exam 3 Chem 1212 Fall 2014 (chapters 3,4, 14,15)
Chapter 3
Nomenclature ionic compounds, molecular compounds, simple organic compounds, hydrates, acids
Know the names and charges of the polyatomic ions
Calculation molecular weight mw
Molar mass of compound
Number particles = NA x n
Mass %
Determination of empirical formula and molecular formula
Combustion analysis
Balancing equations
Chapter 4
Limiting reactant
Mole to mole conversion from reaction stoichiometry
Theoretical yield, Percent yield, Actual yield
Solution concentration (molarity) M = n/V , V always in L
M1V1=M2V2 ( dilution calculations)
Stoichiometry of reactions in solutions M1V1=M2V2 ( dilution calculations)
Ionic reactions (formula unit equation, complete ionic and net ionic equation). Solubility rule
Types of ionic equations: acid-base, precipitation, gas evolution.
Spectator ions
Oxidation-reduction reactions (how to distinguish ox-red reactions vs. ionic equations)
Oxidation, reduction, reducing and oxidizing agent.
Chapter 14
Dynamic Equilibrium and equilibrium constant, expressing Equilibrium constant for chemical reactions
Large and Small equilibrium constant
Relationship between Kc and Kp
Heterogeneous equilibria and Kc or Kp expressions for heterogeneous reactions.
Reaction quotient
Problems: Finding equilibrium constant if concentrations are known, finding equilibrium concentrations if constant is known (ICE table), approximation in solution if K is relatively small and initial concentration is relatively large.
Le Châtelier’s Principle: when a chemical system at equilibrium is disturbed, the system shifts in a direction that minimizes the disturbance
Effect of Concentration, Pressure (Volume) and Temperature Change on equilibrium.
Chapter 15
Classification of Acids and Bases. Acids: Strong, weak, binary, oxyacids, carboxylic acids. Strength of acids depends on structure. Bases: ionic, covalent. Strength of bases.
Definitions of Acids and Bases: the Arrhenius Theory,
Chapter 3
Nomenclature ionic compounds, molecular compounds, simple organic compounds, hydrates, acids
Know the names and charges of the polyatomic ions
Calculation molecular weight mw
Molar mass of compound
Number particles = NA x n
Mass %
Determination of empirical formula and molecular formula
Combustion analysis
Balancing equations
Chapter 4
Limiting reactant
Mole to mole conversion from reaction stoichiometry
Theoretical yield, Percent yield, Actual yield
Solution concentration (molarity) M = n/V , V always in L
M1V1=M2V2 ( dilution calculations)
Stoichiometry of reactions in solutions M1V1=M2V2 ( dilution calculations)
Ionic reactions (formula unit equation, complete ionic and net ionic equation). Solubility rule
Types of ionic equations: acid-base, precipitation, gas evolution.
Spectator ions
Oxidation-reduction reactions (how to distinguish ox-red reactions vs. ionic equations)
Oxidation, reduction, reducing and oxidizing agent.
Chapter 14
Dynamic Equilibrium and equilibrium constant, expressing Equilibrium constant for chemical reactions
Large and Small equilibrium constant
Relationship between Kc and Kp
Heterogeneous equilibria and Kc or Kp expressions for heterogeneous reactions.
Reaction quotient
Problems: Finding equilibrium constant if concentrations are known, finding equilibrium concentrations if constant is known (ICE table), approximation in solution if K is relatively small and initial concentration is relatively large.
Le Châtelier’s Principle: when a chemical system at equilibrium is disturbed, the system shifts in a direction that minimizes the disturbance
Effect of Concentration, Pressure (Volume) and Temperature Change on equilibrium.
Chapter 15
Classification of Acids and Bases. Acids: Strong, weak, binary, oxyacids, carboxylic acids. Strength of acids depends on structure. Bases: ionic, covalent. Strength of bases.
Definitions of Acids and Bases: the Arrhenius Theory,